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General and Physical Chemistry–Syllabus- one Semester Sackler faculty of medicine Tel-Aviv University-Israel CONTENTS: Chemistry and Measurement: Introduction to Chemistry, Matter: Physical State and Chemical Constitution, Measurements, Units. Atoms, Molecules, and Ions: The Structure of the Atom, Isotopes, Atomic Weights, Periodic Table of the Elements, Chemical Substances, Chemical Reactions: Equations. Stoichiometry: Molecular Weight and Formula Weight, The Mole Concept, Mass Percentages from the Formula, Elemental Analysis: Percentages of Carbon, Hydrogen, and Oxygen. Determining Formulas, Molar Interpretation of a Chemical Equation, Amounts of Substances in a Chemical Equation, Limiting Reactant: Theoretical and Percentage Yields. Chemical Reactions: Ionic Theory of Solutions, Molecular and Ionic Equations, Precipitation Reactions, Acid–Base Reactions, Oxidation–Reduction Reactions, Balancing Oxidation–Reduction Equations, Molar Concentration Diluting Solutions, Titration. Gases: Gas Pressure and Its Measurement, Empirical Gas Laws, The Ideal Gas Law, Stoichiometric Relationships with Gases, Gas Mixtures; Law of Partial Pressures, Kinetic Theory of Gases, Molecular Speeds; Diffusion and Effusion. Thermochemistry: Energy and Its Units, First Law of Thermodynamics; Work and Heat, Heat of Reaction; Enthalpy of Reaction, Thermochemical Equations, Applying Stoichiometry to Heats of Reaction, Measuring Heats of Reaction, Hess’s Law, Standard Enthalpies of Formation. Atomic Structure: The Wave Nature of Light, Quantum Effects and Photons, The Bohr Theory of the Hydrogen Atom, Quantum Mechanics, Quantum Numbers and Atomic Orbitals, Electron Spin and the Pauli Exclusion Principle, Building-Up Principle and the Periodic Table, Writing Electron Configurations 3 מתוך1 עמוד Using the Periodic Table, Orbital Diagrams of Atoms; Hund’s Rule, Some Periodic Properties. Chemical Bond: Describing Ionic Bonds, Electron Configurations of Ions, Ionic Radii, Describing Covalent Bonds, Polar Covalent Bonds; Electronegativity, Writing Lewis Electron-Dot Formulas, Formal Charge and Lewis Formulas, Delocalized Bonding: Resonance, Exceptions to the Octet Rule, Bond Length and Bond Order, Bond Energy, The Valence-Shell Electron-Pair Repulsion (VSEPR) Model, Dipole Moment and Molecular Geometry, Valence Bond Theory, Description of Multiple Bonding, Principles of Molecular Orbital Theory, Electron Configurations of Diatomic Molecules of the Second-Period Elements, Molecular Orbitals and Delocalized Bonding. Intermolecular Forces: Comparison of Gases, Liquids, and Solids, Phase Transitions, Properties of Liquids: Surface Tension and Viscosity, Intermolecular Forces; Explaining Liquid Properties, Classification of Solids by Type of Attraction of Units. Chemical kinetics: Definition of Reaction Rate, Experimental Determination of Rate, Dependence of Rate on Concentration, Change of Concentration with Time, Temperature and Rate; Collision and Transition-State Theories, Arrhenius Equation, Reaction Mechanisms: Elementary Reactions, The Rate Law and the Mechanism, Catalysis. Chemical Equilibrium: Chemical Equilibrium—A Dynamic Equilibrium, The Equilibrium Constant, Heterogeneous Equilibria; Solvents in Homogeneous Equilibria, Qualitatively Interpreting the Equilibrium Constant, Predicting the Direction of Reaction, Calculating Equilibrium Concentrations, Removing Products or Adding Reactants, Changing the Pressure and Temperature, Effect of a Catalyst. Acids and Bases: Arrhenius Concept of Acids and Bases, Brønsted–Lowry Concept of Acids and Bases, Lewis Concept of Acids and Bases, Relative Strengths of Acids and Bases, Molecular Structure and Acid Strength, Autoionization of Water, Solutions of a Strong Acid or Base, The pH of a Solution, Acid-Ionization Equilibria, Polyprotic Acids, Base-Ionization Equilibria, Acid–Base Properties of Salt Solutions, Common-Ion Effect, Buffers, Acid–Base Titration Curves. 3 מתוך2 עמוד Colligative Properties: Ways of Expressing Concentration, Vapor Pressure of a Solution, Boiling-Point Elevation and Freezing-Point Depression, Osmosis, Colligative Properties of Ionic Solutions. Free Energy and Spontaneity: Entropy and the Second Law of Thermodynamics, Standard Entropies and the Third Law of Thermodynamics, Free Energy and Spontaneity, Change of Free Energy with Temperature, RelatingG to the Equilibrium Constant, Interpretation of Free Energy. Electrochemistry: Construction of Voltaic Cells, Notation for Voltaic Cells, Cell Potential, Standard Cell Potentials and Standard Electrode Potentials, Equilibrium Constants from Cell Potentials, Dependence of Cell Potentials on Concentration, Some Commercial Voltaic Cells, Electrolysis, Stoichiometry of Electrolysis. Bibliography: 1. Chemistry , Steven S. Zumdahl , Susan A. Zumdahl. 2. General Chemistry: Principles and Modern, Ralph H. Petrucci , F. Geoffrey Herring , Jeffry D. Madura , Carey Bissonnette. 3. General Chemistry, Darrell Ebbing , Steven D. Gammon. 4. Chemistry , John E. McMurry , Robert C. Fay , Jill Kirsten Robinson. 5. Principles of Chemistry: A Molecular Approach, Nivaldo J. Tro. 6. Chemistry: The Molecular Science ,John W. Moore, Conrad L. Stanitski. 7. Chemistry: The Central Science, Theodore E. Brown , H. Eugene LeMay , Bruce E. Bursten , Catherine Murphy, Patrick Woodward , Matthew E. Stoltzfus. 8. Chemistry: Principles and Reactions, William L. Masterton , Cecile N. Hurley. Dr. Haj Yahya Anan 3 מתוך3 עמוד